To calculate the heat required to convert 74 g of ice at -4 °C to 52 °C, we need to know the specific heat capacity of ice and water. We can use the following formula:
q = mcΔT
m = mass of substance
c = specific heat capacity
ΔT = change in temperature
The specific heat capacity of ice is 2.108 J/g°C and for water is 4.187 J/g°C. We will first calculate the heat to convert ice from -4 °C to 0 °C. Then we will calculate the heat to increase the temperature of water from 0 °C to 52 °C.
From -4 °C to 0 °C:
q = (74 g)(2.108 J/g°C)(4°C)
q = 624 J
From 0 °C to 52 °C:
q = (74 g)(4.187 J/g°C)(52°C)
q = 16,112 J
The total heat required to convert 74 g of ice at -4 °C to 74 g of water at 52 °C is the combined calculated heats:
Total heat = 16,112 + 624
Total heat = 16,736 J = 16.7 kJ
The atomic mass of Cs is 132.9. So the mole number of 675 g cesium is 675/132.9 = 5.08 mole. Then the answer should be 5.08 mole.
wind can erode the rock, sunlight can bleach a rock but doesn't affect its shape,water weathers down the rock and ice can form and break of prices of the rock if the ice gets chipped, so I'm guessing sunlight.
Answer:
10.15748 so it is none of the above
Explanation:
I just know
Answer:
24.309 g/mol
Explanation:
To get the atomic mass, all we have to do is calculate with the masses of the three isotope, the real quantity present, taking account of the percent and then, do a sum of these three values. Like a pondered media.
For the first isotope:
23.99 * (78.99/100) = 18.95 g/mol
For the second isotope:
24.99 * (10/100) = 2.499 g/mol
For the last isotope:
25.98 * (11.01/100) = 2.86 g/mol
Now, let's sum all three together
AW = 18.95 + 2.499 + 2.86
AW = 24.309 g/mol
