What mass (in g) of butanol (C4H10O) is required such that its combustion produces 67.4 g of products? The combustion of a compound (containing C, H, and O) is its reaction with molecular oxygen (O2) to produce water and carbon dioxide.
In a 5.00 L steel container at 575 K, the partial pressures of H2(g) and O2(g) are respectively 19.95 and 13.02 atm. The H2(g) and the O2(g) react together to produce H2O(g). The final temperature remains at 575 K and the volume remains at 5.00 L. What is the final total pressure (in atm)?
We have a bomb calorimeter with a heat capacity of 555 J/K. In this bomb calorimeter, we place 1000.0 mL of water. We burn 2.433 g of a solid in this bomb calorimeter. The temperature of the bomb calorimeter and the water increases by 2.30 oC. The molar mass of the solid is 533.5 g/mol. How much heat (in kJ) will be released if we were to burn 0.172 mol of this same solid in the bomb calorimeter? Keep in mind that we want to find the amout of heat released. The specific heat capacity or water is 4.184 J/K/g. Approximate the density of water as being exactly 1.00 g/mL.
The density of a sample of NH3(g) at a pressure of 1.00 atm is 0.931 g/L. What is the root-mean-square speed (in m/s) of the molecules in this sample?
1. 18.75 grams of C4H10O is required to produce 67.4 grams of the products... View the full answer