If 7.50 mol of NH₃ and 6.20 mol of O₂ react in the following reaction, how many moles of H₂O will be formed? 4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g) If 32.0 g of NO and 26.9 g of O₂ react together, what is the mass in grams of NO₂ that can be formed via the reaction below? 2 NO (g) + O₂ (g) → 2 NO₂ (g) When copper is heated with an excess of sulfur, copper(I) sulfide is formed. In a given experiment, 1.50 g of copper was heated with excess sulfur to yield 1.66 g copper(I) sulfide. What is the percent yield? What volume (in mL) of 0.4000 M HCl is required to neutralize 60.00 mL of 0.7000 M KOH? A sample of gas at a constant pressure initially has a temperature of 273.15 K with a volume of 347 mL. The temperature changes to 406.15 K. Calculate the final volume. The volume of a balloon filled with He at 755 mmHg is expanded from 2.20 L to 5.70 L at a constant temperature. What is the final pressure (in atm) of the the balloon? At a constant temperature and pressure, there are initially 1.20 moles of a gas at a volume of 1.25 L. The volume changes to 2.45 L. Calculate the moles of gas in this new volume. In a sealed and rigid container, a sample of gas at 4.40 atm and 60.0 °C is cooled to 20.0 °C. What is the pressure (in atm) of the gas at 20.0 °C? 25.0 L of an ideal gas at 278 K and 4.11 atm are heated to 393 K with a new pressure of 9.60 atm. What is the new volume (in L)? What is the molar mass of an unknown gas with a density of 1.70 g/L at 3.00 atm and 45.0 °C? At 45.0 °C, a 14.00 L vessel is filled with 4.26 atm of Gas A and 5.89 atm of Gas B. What is the mole fraction of Gas B?
If 7.50 mol of NH₃ and 6.20 mol of O₂ react in the following reaction, how many moles of H₂O will be formed? 4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g)
If 32.0 g of NO and 26.9 g of O₂ react together, what is the mass in grams of NO₂ that can be formed via the reaction below? 2 NO (g) + O₂ (g) → 2 NO₂ (g)
When copper is heated with an excess of sulfur, copper(I) sulfide is formed. In a given experiment, 1.50 g of copper was heated with excess sulfur to yield 1.66 g copper(I) sulfide. What is the percent yield?
What volume (in mL) of 0.4000 M HCl is required to neutralize 60.00 mL of 0.7000 M KOH?
A sample of gas at a constant pressure initially has a temperature of 273.15 K with a volume of 347 mL. The temperature changes to 406.15 K. Calculate the final volume.
The volume of a balloon filled with He at 755 mmHg is expanded from 2.20 L to 5.70 L at a constant temperature. What is the final pressure (in atm) of the the balloon?
At a constant temperature and pressure, there are initially 1.20 moles of a gas at a volume of 1.25 L. The volume changes to 2.45 L. Calculate the moles of gas in this new volume.
In a sealed and rigid container, a sample of gas at 4.40 atm and 60.0 °C is cooled to 20.0 °C. What is the pressure (in atm) of the gas at 20.0 °C?
25.0 L of an ideal gas at 278 K and 4.11 atm are heated to 393 K with a new pressure of 9.60 atm. What is the new volume (in L)?
What is the molar mass of an unknown gas with a density of 1.70 g/L at 3.00 atm and 45.0 °C?
At 45.0 °C, a 14.00 L vessel is filled with 4.26 atm of Gas A and 5.89 atm of Gas B. What is the mole fraction of Gas B?
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