When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced. 2 Al(s) + 6 HC1(aq) 2 AICI, (aq) + 3 H, (g) What volume of H, (g) is produced when 7.10 g Al(s) reacts at STP? volume of H, (g):

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

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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)

A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.

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)

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At 1.00 atm and  0 ∘C,  a  5.04 L  mixture of methane  (CH4)  and propane  (C3H8)  was burned, producing  15.7 g CO2.  What was the mole fraction of each gas in the mixture? Assume complete combustion. Xmethane= Xpropane=

(1) - The temperature is 21.3° C, atmospheric pressure is 755 mmHg and the volume of the gas bag is 981 mL. Convert each of these measurements to a set of units needed in the Ideal Gas law. Show all work! i) ii) temperature: pressure: volume:

(ans: -7.50 x 10 ) one mole of sucrose). Imol %3D 9reaction=n AH %3D %3D (ans: -5.64 x 10 kJ/mol) Calcium chloride and sodium hydroxide react according to the equation: CaCl(aq) + 2 NaOH(aq) → Ca(OH),(s) +2 NaCl(aq) What volume of 2.00 M NaOH would be needed to react with 50.0 mL of 1.50 M CaCl,? a, 017 (ans: 75.0 mL) b) When 50.0 mL of 1.50 M CaCl, solution and 80.0 mL of 2.00 M NAOH solution (i.e., 5.0 mL more than calculated in part (a)) both initially at 22.3°C are mixed in a coffee-cup calorimeter with a calorimeter constant of 12.8 J/ C, the temperature fell to 20.0°C. If the density of the reaction mixture is 1.03 g/mL and its specific heat 3.94 J/g°C, calculate the heat absorbed hv the reaction. (ans: 1.24 x 103) c) Calculate AH (in kJ per mole of Ca(OH)2 formed) for the reaction. (ans: 1.6 x 10' kJ/mol)