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3 years ago

Which images show a container holding a heterogeneous mixture?

Chemistry

2 answers:

NeX [460]3 years ago

6 0

Answer:

Explanation:

You can clearly see what is mixed up in the bowl.

Therefore the answer is A

marshall27 [118]3 years ago

4 0

Answer:

Explanation:

a heterogeneous mixture is one that is not uniform in composition.It is made up of non-uniform mix of smaller constituent parts that could be separated from one another using various means.

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A sample of water with a mass of 587.00 kg is heated with 87 kJ of energy to a temperature of 518.4 K. The specific heat of wate

AlladinOne [14]

Answer : Initial temperature of the water is 518.3 K

Explanation :

The specific heat of water (Cp) can be expressed in 2 ways

1) Cp = 1 J g⁻¹ K⁻¹ or

2) Cp = 1 kJ kg⁻¹ K⁻¹

The amount of heat absorbed by water is given by the following equation.

Q = m×Cp×ΔT

Here Q is the amount of energy absorbed in kilojoules

m is the mass of water in kilograms

Cp is specific heat of water

ΔT is the difference is temperature of water.

We have been given that

Q = 87 kJ

Cp = 1 kJ kg⁻¹ K⁻¹

m = 587.00 kg

Let us plug in these values in equation for Q

Q = mxCpxΔT

87 kJ = 587.00 kg x 1 kJ kg⁻¹ K⁻¹ x ΔT

87/587.00 = ΔT

ΔT = 0.15 K

ΔT is calculated as Tf - Ti where Tf is the final temperature and Ti is the initial temperature .

We know that Tf = 518.4 K

And we calculated ΔT as 0.15 K.

Let us plug these values in the equation

ΔT = Tf - Ti

0.15 K = 518.4 K - Ti

Ti = 518.25 K

Initial temperature of the water is 518.3 K

4 0

3 years ago

Which of the following states of matter occurs at the highest temperature?

Aleks [24]

The answer is C. Plasma.

7 0

3 years ago

Read 2 more answers

Prepare a 1.00 L of M solution of sodium carbonate . Determine the amount of sodium carbonate needed incorrect significant figur

Vedmedyk [2.9K]

Answer:b

Explanation:

4 0

4 years ago

A gas has a volume of 4.25 m3 at a temperature of 95.0°C and a pressure of 1.05 atm. What temperature will the gas have at a pre

Goryan [66]

Answer:

$\boxed {\boxed {\sf 82.7 \textdegree C}}$

Explanation:

We are asked to find the temperature of a gas given a change in pressure and volume. We will use the Combined Gas Law, which combines 3 gas laws: Boyle's, Charles's, and Gay-Lussac's.

$\frac {P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

Initially, the gas has a pressure of 1.05 atmospheres, a volume of 4.25 cubic meters, and a temperature of 95.0 degrees Celsius.

$\frac {1.05 \ atm * 4.25 \ m^3}{95.0 \textdegree C}= \frac{P_2V_2}{T_2}$

Then, the pressure increases to 1.58 atmospheres and the volume decreases to 2.46 cubic meters.

$\frac {1.05 \ atm * 4.25 \ m^3}{95.0 \textdegree C}= \frac{1.58 \ atm *2.46 \ m^3}{T_2}$

We are solving for the new temperature, so we must isolate the variable T₂. Cross multiply. Multiply the first numerator by the second denominator, then multiply the first denominator by the second numerator.

$(1.05 \ atm * 4.25 \ m^3) * T_2 = (95.0 \textdegree C)*(1.58 \ atm * 2.46 \ m^3)$

Now the variable is being multiplied by (1.05 atm * 4.25 m³). The inverse operation of multiplication is division, so we divide both sides by this value.

$\frac {(1.05 \ atm * 4.25 \ m^3) * T_2}{(1.05 \ atm * 4.25 \ m^3)} = \frac{(95.0 \textdegree C)*(1.58 \ atm * 2.46 \ m^3)}{(1.05 \ atm * 4.25 \ m^3)}$

$T_2=\frac{(95.0 \textdegree C)*(1.58 \ atm * 2.46 \ m^3)}{(1.05 \ atm * 4.25 \ m^3)}$

The units of atmospheres and cubic meters cancel.

$T_2=\frac{(95.0 \textdegree C)*(1.58* 2.46 )}{(1.05 * 4.25 )}$

Solve inside the parentheses.

$T_2= \frac{(95.0 \textdegree C)*3.8868}{4.4625}$

$T_2= \frac{369.246}{4.4625} \textdegree C}$

$T_2 = 82.74420168 \textdegree C$

The original values of volume, temperature, and pressure all have 3 significant figures, so our answer must have the same. For the number we calculated, that is the tenths place. The 4 in the hundredth place to the right tells us to leave the 7 in the tenths place.

$T_2 \approx 82.7 \textdegree C$