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Consider the following reaction in a closed reaction flask. If 1.50 atm of gas A is allowed to react with 0.500 atm of gas B and the reaction goes to completion at constant temperature and volume, what is the total pressure in the reaction flask at the end of the reaction? What are the partial pressures of the gases in the flask?
4A(g) + 6B(g) ? 2A2B3(g)
A. (0.750 atm A2B3 produced) + (0.25 atm B remaining) = 1.00 atm total pressureB. (0.167 atm A2B3 produced) + (1.17 atm A remaining) = 1.34 atm total pressureC. (1.50 atm A2B3 produced) + (0.167 atm A remaining) = 1.67 atm total pressureD. (0.333 atm A2B3 produced) + (0.500 atm A remaining) = 0.833 atm total pressure
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given the reaction 4als 3o2g --gt 2al2o3s what is the minimum number of moles of oxygen gas required to produce 1.00
starting with an aqueous solution of 115 ml of 0.35 m pyridine kb 1.7 x 10-9 determine the observed ph of the solution
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