This is a PV=nRT problem, commonly known as ideal gas. For this, we simply need to take what we know and plug it into the equation
Pressure x Volume = moles x ideal gas constant x tempature.
We know our pressure is 589mmHg so we can plug that in. The volume is unknown.
Then, we need to convert 8.45g of CO2 to moles. That is the grams to moles stoichiometry problem. I will not solve the problem for you, however I can set it up for you:
8.45gCO2 1 mole CO2
-------------- x --------------
1 44.01g CO2
At this point, we now have 589 x X= moles.
The ideal gas constant for mmHg should have been given to you, it is 62.4.
Then, we need to convert from celcius to kelvin. To do this, we simply add 273 to 10, since 273 is the standard unit for kelvin.
Now that we have all of our units, we can plug them into the PV=nRT formula, and solve. We are finding the V, so therefore to find it, the P (pressure) needs to equal the nRT. We would multiple nRT together to get an answer, and divide by the pressure to get the missing unit. To make sure you got the right answer, multiply P and V together to see if it equals nRT. And don't forget to round to the least number of sig figs! Hope I could be of help!
Answer:
I think the answer might be D. but im not 100 percent sure
Explanation:
Answer:
The best definition is: "Buffer capacity is the amount of acid or base that can be added to a buffer without destroying its effectiveness"
Explanation:
A buffer is a solution that is somewhat resist to pH changes by reacting with acids and bases that may be added into the solution. It's capacity is the amounto of acid or base that can be added into solution without much change in pH.
So the best definition is: "Buffer capacity is the amount of acid or base that can be added to a buffer without destroying its effectiveness"
Answer:
True
Explanation:
The more of each substanse that you add to the bag will cause it to produce faster and more gas.
