1&2 Use the ideal gas law to derive the combined gas law. Assuming so elasticity
ID: 967358 • Letter: 1
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1&2 Use the ideal gas law to derive the combined gas law. Assuming so elasticity forces in rubber, what volume should a 1.0 L balloon at 25 degree C and 1.00 atmosphere pressure be if immersed in liquid nitrogen (-196 degree C, 1 atm)? When this experiment is actually performed, the volume of the balloon approaches 0.0 L. How do you account for the discrepancy? 0.525 grams of magnesium is reacted with an excess amount of aqueous hydrochloric acid at 27 degree C and 752 mm_Hg. Calculate the number of moles of hydrogen gas produced and its volume under the above conditions. Climate change is a topic of considerable discussion. In order to have an understanding of the science of climate change, it is necessary to have some knowledge of the gases present in our atmosphere. Write down what you think are the three most abundant gases in the atmosphere (not counting water vapor which varies from 0% to 4%). Now look up the atmospheric content (do not change your original answer as you will not lose points for being wrong) and record the names of the four most abundant gases and their percentages. There is a follow-up exercise to this in Activity 35 in Part B, #1. Most abundant gases in the atmosphere (excluding water vapor)Explanation / Answer
1) Ideal gas equation is :- P*V = n*R*T
Now, when moles of the gas is constant,
P*V/T = constant
Thus, P1*V1/T1 = P2*V2/T2 which is the combined gas law.
3) Mg(s) + 2HCl(aq) ----> MgCl2 + H2(g)
Molar mass of Mg = 24 g/mole
Moles of Mg in 0.525 g of it = mass/molar mass = 0.0219
Thus, moles of H2 produced = moles of Mg reacted = 0.0219
Applying Ideal Gas Equation we get,
Volume of H2 produced, V = n*R*T/P = 0.0219*0.0821*300/(752/760) = 0.544 litres = 544 ml
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