The main objective of this lab was to collect 〖Co〗_2 gases that were given off by the Alka-Seltzer tablets and to identify experimental masses. The volume of gas was 724 liters, or 723.86 cm and the experimental mass was .0894 grams. A balance scale was used before and after the reaction to record the change in overall mass. First, using the scale, the flask, balloon, and Alka-Setlzer tablets were measured, 259.4 ±.05 Grams were found. What created the “〖Co〗_2 gases to be trapped” were the crushed Alka-Seltzer tablets that went into the flask that contained water. The balloon that was attached to the flask was able to contain the 〖Co〗_2 that’s pressure was pushing forward, which helps one infer the rate of the chemical reaction. Throughout
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The 35 centimeters, the “border”, played a huge part in finding the volume of gas produced. By diving the 35 cm by 2 π, the radius was found. The radius, 5.57 cm, was plugged into the equation (4⁄(3 ) π)(〖5.57)〗^3 to give the answer 723.86 〖cm〗^3. Whats also important to point out is this needs to be converted into liters, and then it’s 724 liters. The ideal gas law, PV=nRT, was a formula that determined the number of moles produced. Taking the Barometric pressure, 769.9mmHg, and subtracting it from the volume of water, 17.5 mmHg, can formulate the pressure. Since pressure is what’s needed, 752.4 had to be divided by 760 to be converted into atm creating 0.99atm. Then with plugging in the rest, using .0821 and (20+273), the number of moles can be found by getting n, moles, alone. The answer then is .0298 moles of gas produced. After the reaction, and an incision to release the gas, the mass also had to be identified, which was less than the previous mass, 255.9 grams. The experimental molar mass was 0.0894 grams, found by using the moles of 〖Co〗_2 and the masses. The percent yield came about by dividing the experimental molar mass by the theoretical (44.01grams) to create 20 percent. The percent yield shows how far off the experimental calculations were from the truth. Overall, by using the Alka-Seltzer, what could be concluded was that Alka-Seltzer reacts
The 35 centimeters, the “border”, played a huge part in finding the volume of gas produced. By diving the 35 cm by 2 π, the radius was found. The radius, 5.57 cm, was plugged into the equation (4⁄(3 ) π)(〖5.57)〗^3 to give the answer 723.86 〖cm〗^3. Whats also important to point out is this needs to be converted into liters, and then it’s 724 liters. The ideal gas law, PV=nRT, was a formula that determined the number of moles produced. Taking the Barometric pressure, 769.9mmHg, and subtracting it from the volume of water, 17.5 mmHg, can formulate the pressure. Since pressure is what’s needed, 752.4 had to be divided by 760 to be converted into atm creating 0.99atm. Then with plugging in the rest, using .0821 and (20+273), the number of moles can be found by getting n, moles, alone. The answer then is .0298 moles of gas produced. After the reaction, and an incision to release the gas, the mass also had to be identified, which was less than the previous mass, 255.9 grams. The experimental molar mass was 0.0894 grams, found by using the moles of 〖Co〗_2 and the masses. The percent yield came about by dividing the experimental molar mass by the theoretical (44.01grams) to create 20 percent. The percent yield shows how far off the experimental calculations were from the truth. Overall, by using the Alka-Seltzer, what could be concluded was that Alka-Seltzer reacts