You set up a reaction with Gallium metal in excess hydrochloric acid at 28 degrees Celsius. It reacts in the following: 2Ga(s)+6HCl(aq)→2GaCl3(aq)+3H2(g) You collect 171 mLs and 0.996 atm of hydrogen over water. How many moles of Ga reacted? The partial pressure of water at 28 degrees is 0.0372 atm.   Rember sig figs

Q: Sodium metal reacts with water to produce hydrogen gas: 2Na(s) + 2H2O(l)2NaOH(aq) + H2(g) In one…

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Q: Calculate the volume of the sample ar constont

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Q: Ammonia, NH3, is formed in the following reaction N2(g) + 3H2(g) → 2NH3(g) N2 and H2 where…

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Q: Consider the following equation: CH&O7(s) +3 NaHCO3(s) + H20(1) --> Na3CgHgO7(s) + 3H2O(1) + 3CO2g)…

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Q: You set up a reaction with Gallium metal in excess hydrochloric acid at 28 degrees Celsius. It…

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A: We have 2 C57H110O6 + 163 O2 → 114 CO2 + 110H2O

Q: All parts of question 2 will walk you through how to calculate the total pressure after the reaction…

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Q: Consider the reaction between solid zinc and hydrochloric acid where hydrogen gas is collected over…

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Q: The following reaction is used to generate hydrogen gas in the laboratory. If 340.6 mL of gas is…

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Q: When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced. 2 Al(s) + 6…

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Q: 2 A 10.5 mL sample of liquid ethanol (C,H,OH, density = 0.789 g/mL) was injected into a 10.0 L…

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Q: A student decomposed 6.900 g of solid ammonium nitrite (MW = 64.04 g/mol) at a temperature of 30.00…

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Q: A sealed can of your favorite soda has a carbon dioxide gas (CO2) volume of .05 L. When it is…

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Q: 16.0 g of KO2 was reacted with CO2 in a 3.00-L tank according to the reaction below. 4 KO2 (s) + 2…

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Q: A sample of magnesium metal reacts completely with an excess of hydrocholoric acid: Mg(s) + 2…

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Q: The balanced equation for the decomposition of potassium chlorate is shown below. When carried out…

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A: The reaction:  2KClO3(s) ==> 2 KCl (s) + 3O2 (g)  Given data :  Total pressure = 755.3 torr…

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Q: A sample of gas contains 0.1700 mol of N2(g) and 0.5100 mol of H2(g) and occupies a volume of 34.1…

A: Avogadro's Law:  At constant temperature and pressure the volume of the gas is directly…

Q: A 2.20 L container at 53.6 °C contains 6.21 g of N2O3(g). The N2⁢O3 gas decomposes completely,…

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Q: 1. Calculate the number of grams of sodium used in the reaction. (The vap 7 0°C =0035? atm )

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Q: A student weighs out 0.0422 g of magnesium metal. The magnesium metal is reacted with excess…

A: The balanced reaction of Mg with HCl is as follows: Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g) Calculation of…

Q: When heated, potassium chlorate decomposes to potassium chloride and oxygen gas according to the…

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Q: A sealed can of your favorite soda has a carbon dioxide gas (CO2) volume of 0.05 L. When it is…

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Q: 5. A student conducts a laboratory investigation of anaerobic respiration. The student places 10.0 g…

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Q: 11. In the presence of a catalyst, potassium chlorate decomposes and provides a very simple way to…

A: Given;

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Q: iron (s) + chlorine (g) →→→→→→ iron(III) chloride (s) grams iron

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Q: You set up a reaction with Gallium metal in excess hydrochloric acid at 28 degrees Celsius. It…

A: The balanced reaction taking place is given as, => 2 Ga (s) + 6 HCl (aq) ---------> 2 GaCl3…

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Q: In the Alka-Seltzer reaction, 19.76 mL of carbon dioxide are measured.  The partial pressure of…

A: The expression of ideal gas equation is shown below: PV = nRT Where; P = pressure V = volume n =…

Q: According to the reaction below, how many grams of sodium chloride can be produced from 31.9 L of…

A: Given: Volume is 31.9 L. Pressure is 0.922 atm. Temperature is 62oC. 2Na+Cl2→2NaCl

Q: MISSED THIS? Read Section 6.7 (Pages 235-238); Watch IWE 6.12. Carbon monoxide gas reacts with…

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Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.