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3 years ago

You have 16.6 g of water at 40.2 C. How many Joules are needed to warm the water to 44.8 C?

Chemistry

1 answer:

iragen [17]3 years ago

3 0

Answer:

Q = 319.49 J

Explanation:

Given that,

Mass, m = 16.6 g

Initial temperature, $T_i=40.2^{\circ} C$

We need to find the heat needed to warm the water to 44.8 °C. The formula that is used to find the heat required is given by :

$Q=mc\Delta T\\\\Q=mc(T_f-T_i)\\\\Q=16.6\ g\times 4.184\ J/g^{\circ} C\times (44.8-40.2)^{\circ} C\\\\Q=319.49\ J$

So, 319.49 J of heat is needed to warm water.

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3 years ago

The density of copper metal is 8.9 g/mL. What is the volume of 2.5 kg of this metal?

AlekseyPX

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Density is directly proportional to mass and inversely proportional to the volume. The density formula is:

$D=\frac{M}{V}$

where D stands for density, M stands for mass and V stands for volume.

Since, the problem asks to calculate the volume, let's rearrange the formula for volume.

$V=\frac{M}{D}$

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The conversion factor is, 1kg = 1000g

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= 2500g

Let's plug in the values in the density formula to calculate the volume.

$\frac{2500g}{\frac{8.9g}{mL}}$

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If the sig figs are considered then the answer needs to be round to two sig figs and hence the volume becomes 280 mL.

8 0

4 years ago

How to find formula for ionic compounds.

Umnica [9.8K]

Answer:

I am using an example for this in this table it works for any other compound as well.

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3 years ago

If a chemical is oxidized it is also known as the

RUDIKE [14]

Answer:

D.) reducing agent

Explanation:

Oxidized chemicals gain electrons. In order to gain these electrons, another chemical must lose electrons. So, the chemical (which will be oxidized) acts as a reducing agent, causing the other chemical to be reduced and lose electrons.

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2 years ago

Which of the following reasons (specific to this lab) would have caused the percent yield of calcium carbonate to be less than 1

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Answer:

Some of the calcium carbonate remained stuck to the side of the glassware after filtering

Some of the calcium carbonate spilled when measuring its mass

Explanation:

The percent yield is obtained from;

Actual yield/Theoretical yield * 100

Usually, the actual yield is less than the theoretical yield thereby making the percent yield less than 100%.

In the case of this particular reaction; when some calcium carbonate remains stuck on the glassware or some calcium carbonate is spilled during weighing, the actual yield of product obtained from the reaction becomes less than the theoretical or calculated yield hence the percent yield becomes less than 100%.

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3 years ago