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Reptile [31]
3 years ago
11

A bowl containing 150 grams of water, is heated from 25 °C to 100 °C. The specific heat of water is 4.184 J/g°C. How much heat e

nergy is required to heat the water?
Chemistry
1 answer:
lyudmila [28]3 years ago
7 0

Answer:

4.7 × 10⁴ J

Explanation:

Step 1: Given data

  • Mass of water (m): 150 g
  • Initial temperature: 25 °C
  • Final temperature: 100 °C
  • Specific heat capacity of water (c): 4.184 J/g.°C

Step 2: Calculate the temperature change (ΔT)

ΔT = 100 °C - 25 °C = 75 °C

Step 3: Calculate the heat required (Q) to raise the temperature of the water

We will use the following expression.

Q = c × m × ΔT

Q = 4.184 J/g.°C × 150 g × 75 °C = 4.7 × 10⁴ J

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As a seed plant grows, the roots grow downward due to the force of​
Rudiy27

Answer:

As a seed plant grows, the roots grow downward due to the force of​  Gravity

Explanation:

A seed is planted upside-down, but the roots still grow in the direction of gravity.

7 0
3 years ago
Calculate the pressure of 2 mol of a gas at 300 K in 8 L container.
Sergio039 [100]

Answer:

4800

Explanation:

using my Cal ex to solve the question

calculation goes like this

2*300*8=4800

3 0
3 years ago
At the boiling point, the vapor pressure of a liquid is equal to the _______.
Marat540 [252]
At the boiling point, the vapor pressure of a liquid is equal to the atmospheric pressure.
6 0
3 years ago
A 17.6-g sample of ammonium carbonate contains ________ mol of ammonium ions.
postnew [5]
These problems are a bit interesting. :)

First let's write the molecular formula for ammonium carbonate. 

NH4CO3 (Note! The 4 and 3 are subscripts, and not coefficients)

17.6 gNH4CO3

Now to convert to mol of one of our substances we take the percent composition of that particular part of the molecule and multiply it by our starting mass. This is what it looks like using dimensional analyse. 

17.6 gNH4CO3 * (Molar Mass of NH4 / Molar Mass of NH4CO3)

Grab a periodic table (or look one up) and find the molar masses for these molecules! Well. In this case I'll do it for you. (Note: I round the molar masses off to two decimal places)

NH4 = 14.01 + 4*1.01 = 18.05 g/mol
NH4CO3 = 14.01 + 4*1.01 + 12.01 + 3*16.00 = 78.06 g/mol


17.6 gNH4CO3 * (18.05 molNH4 / 78.06 molNH4CO3)
= 4.07 gNH4

Now just take the molar mass we found to convert that amount into moles!

4.07 gNH4 * (1 molNH4 / 18.05 gNH4) = 0.225 molNH4

4 0
3 years ago
Solid silver chloride, AgCI(s), decomposes to its elements when exposed to sunlight Write a balanced equation for this reaction
Mrac [35]

Answer: The coefficient in front of AgCl when the equation is properly balanced is 2.

Explanation:

According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

Decomposition is a type of chemical reaction in which one reactant gives two or more than two products.

Decomposition of silver chloride is represented as:

2AgCl(s)\rightarrow 2Ag(s)+Cl_2(g)

Thus the coefficient in front of AgCl when the equation is properly balanced is 2.

8 0
4 years ago
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