Multiple Choice
Why should a zeotropic refrigerant not be charged into a refrigeration system in vapor form?
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7. Gases
Gas Stoichiometry
Multiple Choice
Determine the mass (in grams) of water formed when 15.3 L NH3 (at 298 K and 1.50 atm) is reacted with 21.7 L of O2 (at 323 K and 1.1 atm).
4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g)
A
12 g
B
19 g
C
25 g
D
38 g
E
51 g
Verified step by step guidance1
First, use the ideal gas law to calculate the number of moles of NH3. The ideal gas law is given by the equation: , where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.
Calculate the number of moles of NH3 using the given conditions: P = 1.50 atm, V = 15.3 L, and T = 298 K. Rearrange the ideal gas law to solve for n: .
Next, calculate the number of moles of O2 using the ideal gas law with the given conditions: P = 1.1 atm, V = 21.7 L, and T = 323 K. Use the same rearranged formula: .
Determine the limiting reactant by comparing the mole ratio of NH3 to O2 from the balanced chemical equation: 4 NH3 + 5 O2 → 4 NO + 6 H2O. Calculate the theoretical moles of water produced by each reactant and identify the limiting reactant.
Finally, use the stoichiometry of the balanced equation to calculate the mass of water formed. The balanced equation shows that 4 moles of NH3 produce 6 moles of H2O. Use the molar mass of water (18.02 g/mol) to convert moles of water to grams.
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