Answer:
We need 420 cal of heat
Explanation:
Step 1: Data given
Mass of the aluminium = 200.0 grams
Temperature rises with 10.0 °C
Specific heat of aluminium = 0.21 cal/g°C
Step 2: Calculate the amount of heat required
Q =m * c* ΔT
⇒with Q = the amount of heat required= TO BE DETERMINED
⇒with m = the mass of aluminium = 200.0 grams
⇒with c = the specific heat of aluminium = 0.21 cal/g°C
⇒with ΔT = the change of temperature = 10.0°C
Q = 200.0 grams * 0.21 cal/g°C * 10.0 °C
Q = 420 cal
We need 420 cal of heat (option 2 is correct)
<span>the solvent, hope this helps</span>
Answer:
1.18 moles of gas
Explanation:
3.00 moles of gas are pumped into a 1.00L rigid container with a pressure of 1.98 atm. The gas is released from the container until the pressure is 0.78 atm, how many moles of gas remain in the container?
for the sealed rigid container, the pressure is directly proportional to the amount of gas
3.00moles/1.98 atm = ? moles/0.78 atm
? = 3.00 X 0.78/1.98 =1.18 moles of gas
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