How many joules are absorbed when 64.3 grams of water is heated from 40.0 °C to 74.0 °C?

Chemistry

2 answers:

REY [17]3 years ago

6 0

Answer : The correct option is, (B) 9150 joules

Explanation : Given,

Initial temperature = $40.0^oC$

Final temperature = $74.0^oC$

Mass of water = 64.3 g

Specific heat of water = $4.184J/g^oC$

Formula used :

$Q=m\times C_w\times \Delta T$

or,

$Q=m\times C_w\times (T_2-T_1)$

where,

Q = heat absorbed = ?

m = mass of water

$C_w$ = specific heat of water

$T_1$ = initial temperature

$T_2$ = final temperature

Now put all the given value in the above formula, we get:

$Q=64.3g\times 4.184J/g^oC\times (74-40)^oC$

$Q=9150J$

Therefore, the heat absorbed will be, 9150 J

Alinara [238K]3 years ago

3 0

D dhdidisknfucuenfhdienxjxidondhdjjeixjndi

You might be interested in

What's the amount of solute in 1.75 L of 0.25 M HCl?

Fynjy0 [20]

Answer: 0.4375 mols of solute

Explanation:

The problem is asking for the amount of solute. We are given the value of molarity. The molarity is 0.25M. We know that molarity is $M=\frac{mols of solute}{liters of solution}$ . Since we are given the liters of solution is 1.75, we can use those values to solve for mols of solute.