Answer:
Explanation:
Hello!
In this case, since the first law of thermodynamics allows us to understand how the energy behaves when heat and work are involved during a process, we can mathematically define it as:
Whereas Q is the heat added to the system, W the work done by the system and ΔU the change in the internal energy, we can notice that since 97.0 J of work are done on the system it would be negative and the given off heat is also heat due to the used convention; therefore the change in its internal energy turns out:
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Answer:
grams/mol of carbon is needed to react with hydrogen gas to produce 59.8 grams of acetylene (C2H2)
Explanation:
The molecular weight of acetylene is 26.04 g/mol
Molecular weight of carbon is equal to 12.011 g/mol
Two carbon atom produces one acetylene molecule.
Thus, 2 * 12.011 g/mol of carbon is used to produce 26.04 g/mol of acetylene,
Amount of carbon required to produce 59.8 grams of acetylene
grams/mol
grams/mol of carbon is needed to react with hydrogen gas to produce 59.8 grams of acetylene (C2H2)
1000 milligrams = 1 gram
Lethal Dose:
10 grams = 10,000 milligrams
Step 1:
Lethal dose divided by mg per can.
10,000 mg / 1.71 mg= 5847.95 ounces
Step 2:
5847.95 oz / 12 oz per can= 487.32 cans
Step 3:
Round up to 488 cans because we have to buy whole cans.
Hope this helps! :)