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Calculate the amount of heat needed to boil 113. g of water (H,0), beginning from temperature Of 4.4 "C_ Round your answer t0 significant digits_ Also, sure yo...

Question

Calculate the amount of heat needed to boil 113. g of water (H,0), beginning from temperature Of 4.4 "C_ Round your answer t0 significant digits_ Also, sure your answer contains unit symbol:Oo

Calculate the amount of heat needed to boil 113. g of water (H,0), beginning from temperature Of 4.4 "C_ Round your answer t0 significant digits_ Also, sure your answer contains unit symbol: Oo



Answers

Calculate the amount of heat (in $\mathrm{kJ}$ ) required to convert $74.6 \mathrm{g}$ of water to steam at $100^{\circ} \mathrm{C}$.

The amount of heat is equal to specific heat multiplied with mass multiplied with temperature change. So specific heat is 4.184 jules. Program degree Celsius, Mass is 55.2 g And the change in temperature 30 And the changes temperature is 17°C 30 to -15°C simply. And the amount of heat is three 96 point 266 Chul's, which can also be written as 3.9 3.93 10 days to power three tools. This is the amount of heat needed to raise 55.2 g of water at 17.

Good day. This question. We will be converting the temperature in Fahrenheit to temperature in sell shoes using the equation that we got, which is Temperature in solutions is equal to 5.9. I have a temperature in Fahrenheit -32. We can solve the degree in Fahrenheit 2°. Our shoes substituting, we have 5 4.9 Times 212 -32. Computing, we will get temperature in solutions is equal to 100 degree sociales. Thank you.

We used the heat equation dancer This question were que is going to be equal to the specific keep multiplied by the mass multiplied by the change in temperature. So we have Q b unequal Do the specific it of water 4.184 jewels per gram degree Celsius multiplied by the mass of 65 g, will play by the change in temperature, which will be the final temperature 65 minus the initial 32 and we get 9000 jewels.

Question 80 is pretty straightforward. It simply ask you to calculate the amount of heat in Kila jewels there just required to convert a certain mass 152 point grams of water to steam at 100 degrees Celsius. So we're already at 100 degrees Celsius and any energy that we add into 152 point grams of water is going to convert it into steam. And we just want to convert all of it thio steam while maintaining the temperature of 100 degrees Celsius. So all we need is the Delta H, uh, vaporization for the calculation in this problem. So we have 152 150.2 g of water, which we can convert two moles. Then when we have moles of water, we can use the Delta H, uh vaporization of water, which you can look up in your textbook. His 40.79 killer jewels per mole and we get 340 point to kill the jewels of energy required to convert 150.2 g of water at 100 degrees Celsius to steam at 100 degrees Celsius.


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