Answer:
Hey hi
Explanation:
Can you pls tell me which language is this pls I really want to help you... Sorry
Answer:
Q = 2647 J
Explanation:
Specific heat capacity is the amount of energy required by one Kg of a substance to raise its temperature by 1 °C.
In thermodynamics the equation used is as follow,
Q = m Cp ΔT
Where;
Q = Heat = ?
m = mass = 660 g
Cp = Specific Heat Capacity = 0.3850 J.g⁻¹.°C⁻¹
ΔT = Change in Temperature = 23.35 °C - 12.93 °C = 10.42 °C
Putting values in eq. 1,
Q = 660 g × 0.3850 J.g⁻¹.°C⁻¹ × 10.42 °C
Q = 2647 J
Answer:
im not sure
Explanation:
i went on here looking nobody answered yet
Answer:
When two or more atoms chemically bond with each other, the resultant chemical structure is a molecule. The familiar water molecule, H2O, consists of two hydrogen atoms and one oxygen atom; these bond together to form water, irdk but it's either C or D
Explanation:
hope this helps have a good rest of your day :) ❤
The enthalpy change for melting ice is called the entlaphy of fusion. Its value is 6.02 kj/mol. This means for every mole of ice we melt we must apply 6.02 kj of heat. We can calculate the heat needed with the following equation:
Q = N x ΔH
where:
Q = heat
N = moles
ΔH = enthalpy
In this problem we would like to calculate the heat needed to melt 35 grams of ice at 0 °C. This problem can be broken into three steps:
1. Calculate moles of water
2. multiply by the enthalpy of fusion
3. Convert kJ to J.
Step 1 : Calculate moles of water
![[ 75g ] x (\frac{1 mol}{18.02g} ) =](https://tex.z-dn.net/?f=%5B%2075g%20%5D%20x%20%28%5Cfrac%7B1%20mol%7D%7B18.02g%7D%20%29%20%3D)
Step 2 : Multiply by enthalpy of fusion
Q = N × ΔH = <em> [ Step 1 Answer ]</em> × 6.02 =
Step 3 : Convert kJ to J
![[ Step 2 Answer ] x (\frac{1000j}{1kJ} ) =](https://tex.z-dn.net/?f=%5B%20Step%202%20Answer%20%5D%20x%20%28%5Cfrac%7B1000j%7D%7B1kJ%7D%20%29%20%3D)
Finally rounding to 2 sig figs (since 34°C has two sig figs) we get
Q Would Equal ____