T9 When 1.836 L of 6.000 M hydrochloric acid react with 25.0 g iron how many liters of hydrogen gas form at 25.0°C and 1.00 atm? This and the next question use the reaction: 2 Fe (s) + 6 HCI (aq) → 2 FeCl3 (aq) + 3 H2 (g)

2 H3PO4(s) --> 3 H2(g) + 2 P(s) + 4 O2(g) Using the reaction above, show step by step how many liters of oxygen can be created if I start with 0.7156 grams of H3PO4 solid at STP?

7.78 18) How many grams of zinc metal are required to produce 2.00 liters of hydrogen gas at STP 24.5 Zn(s) + 2 HCl(aq) A) 0. 171 g according to the chemical equation shown below? → ZnCl2(aq) + H2(g) C) 5.83 g B) 131 g D) 11.7 g any to raise the temperature of 53.8 g benzene by

4. At 5°C and 1 atm, x L of O2 gas is required to react with 0.51 g of glucose, what is the value of x? The unbalanced reaction is shown below: C6H12O6 (s) + O2(g) → CO2(g) + H2O(l)

How many grams of Magnesium Oxide form when 14.8L of oxygen gas, measured in STP, completely reacts with Magnesium metal in accordance with the following reaction : 2MgO (s) + O2 (g) = 2MgO (s)

Solid ammonium chloride, NH4Cl, is formed by the reaction of gaseous ammonia, NH3, and hydrogen chloride, HCl. NH3(g)+HCl(g)⟶NH4Cl(s)  A 3.52 g sample of NH3 gas and a 3.52 g sample of HCl gas are mixed in a 2.00 L flask at 25 ∘C. Identify the limiting reagent. NH4Cl   HCl   NH3   How many grams of NH4Cl will be formed by this reaction? What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH4Cl produced by the reaction. ?=

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You are given the balanced equation: C3H8 + 5 02 3 CO2 + 4 H20 If 0.3618 moles of CaHg are allowed to react with 1.818 moles of O2, and this is the only reaction which occurs, what is the theoretical yield of water (in moles) that could be produced? O 1.456 moles O 1.447 moles O 2.180 moles . O 1.454 moles

T8 When 1.836 L of 6.000 M hydrochloric acid react with excess iron how many liters of hydrogen gas form at 25.0°C and 1.00 atm? This and the next 2 questions use the reaction: 2 Fe (s) + 6 HCI (aq) → 2 FeCl3 (aq) + 3 H2 (g) Select one: a. 0.5637 mol b. 0.03132 mol C. none of these d. 0.09395 mol e. 16.4 L f.5.508 mol g. 0.1879 mol h. 135 L

Consider the reaction shown below: 2 HCl (aq) + CaCO3 (s) ⟶ CO2 (g) +  CaCl2 (aq) + H2O (l) How many grams of CaCO3 would need to be consumed to fill a 908.001 mL balloon with CO2 gas, assuming a constant temperature of 21.7 oC and constant pressure of 0.958 atm? Express your answer in units of grams using at least three significant figures.