The following reaction forms 17.3g of Ag(s): What total volume of gas forms if i
ID: 615249 • Letter: T
Question
The following reaction forms 17.3g of Ag(s):
What total volume of gas forms if it is collected over water at a temperature of 25 degrees C and a total pressure of 756mmHg?
Explanation / Answer
The chemical equation is 2 Ag2O(s) ---> 4 Ag(s) + O2(g) states the STOCHIOMETRIC PROPORTION Ag : O2 = 4 : 1 existing among Chemical Products which are Chemical Elements itselves. Since IT HAS BEEN RESCUED A SILVER MASS EQUAL TO 17.3 / 107.8 = 0.16 g mol of Ag CORRENSPONDING TO 0.16 / 4 = 0.04 mol of O2 BY IDEAL GAS, I MAY CORRELATE MOLE GAS-NUMBER OF OXYGEN TO VOLUME IT OCCUPIES OVER WATER p * V = n * R * T where "p" is Gas pressure "V" is occupied volume "n" is mole gas number "R" is Universal Gas Constant "T" is Centigrad Degree Temperature So, I MAY CALCULATE OCCUPIED VOLUME V = n * R * T / p = 0.04 * 0.0821 * (25 + 273.16) / (765 / 760) = = 0.98 Liter
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