If the reaction consumes (uses up) 31.7 moles of ammonia, how many grams of water will be produced using the following equation?
4NH3 + 5O2 g 4NO + 6H2O
If the reaction consumes (uses up) 31.7 moles of ammonia, how many grams of water will...
How many grams of H2O can be prepared from 11.25grams of NH3 and 56.03g of O2in the following equation? 4NH3(g) + 5O2(g) arrow 4NO+ 6H2O(g)
1. How many moles of MgS2O3 are in 225 g of the compound? 2. Determine the empirical formula for a compound that is 64.8% C, 13.6% H, and 21.6% O by mass. 3.A compound is 54.53% C, 9.15% H, and 36.32% O by mass. What is its empirical formula? 4.The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted...
1) Ammonia, NH3, reacts with molecular oxygen, O2, to form nitric oxide, NO, and water:4NH3(g) + 5O2(g) = 4NO (g) +6H2O(l)A. What is the limiting reactant and what is the theoretical yield of NO?B. What is the theoretical yield of H2O?C. How many grams of excess reagent will be left over?D. If the actual yield of NO had been 91 g, what would be the percent yield of the reaction
How many grams of NO and of H2O form? Enter your answers numerically separated by a comma. How many grams of the excess reactant remain after the limiting reactant is completely consumed? One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4NH3(g)+5O2(g)→4NO(g)+6H2O(g) In a certain experiment, 1.50 g of NH3 reacts with 2.75 g of O2.
From the following balanced equation, 4NH3(g)+5O2(g)⟶4NO(g)+6H2O(l) how many grams of NO can be formed from 3.78g O2? Options: (a) 2.55g (b) 2.84g (c) 4.43g (d) 5.04g
One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4NH3(g)+5O2(g)→4NO(g)+6H2O(g) In a certain experiment, 1.85 g of NH3 reacts with 3.39 g of O2. 1) How many grams of NO and of H2O form? 2) How many grams of the excess reactant remain after the limiting reactant is completely consumed?
Nitrogen dioxide reacts with water to produce oxygen and ammonia: 4NO2(g)+6H2O(g)→7O2(g)+4NH3(g) How many grams of NH3 can be produced when 4.10 L of NO2 reacts at 385 ∘C and 735 mmHg ?
One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4NH3(g)+5O2(g)→4NO(g)+6H2O(g) In a certain experiment, 2.05 g of NH3 reacts with 3.76 g of O2. How many grams of NO and of H2O form? Enter your answers numerically separated by a comma.
1. Ammonia reacts with oxygen according to the equation 4NH3(g)+5O2(g)→4NO(g)+6H2O(g),ΔHrxn=−906 kJ Calculate the heat (in kJ) associated with the complete reaction of 155 g of NH3. 2. What mass of butane in grams is necessary to produce 1.5×103 kJ of heat? What mass of CO2 is produced? Assume the reaction to be as follows: C4H10(g)+132O2(g)→4CO2(g)+5H2O(g),ΔHrxn=−2658 kJ
Part A Ammonia reacts with oxygen according to the equation 4NH3(g)+5O2(g)→4NO(g)+6H2O(g),ΔHrxn=−906 kJ Calculate the heat (in kJ) associated with the complete reaction of 155 g of NH3. Part B What mass of butane in grams is necessary to produce 1.5×103 kJ of heat? What mass of CO2 is produced? Assume the reaction to be as follows: C4H10(g)+132O2(g)→4CO2(g)+5H2O(g),ΔHrxn=−2658 kJ