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vivado [14]
2 years ago
11

Use the pie section above to answer this question.

Chemistry
1 answer:
egoroff_w [7]2 years ago
4 0
The answer is Liquid iron.
You might be interested in
Rock transfers heat rapidly.truefalse
MaRussiya [10]
No, it does not. I believe it's false. 
6 0
2 years ago
Suppose 12.0 g of carbon (c) reacts with 70.0 g of sulfur (s) to give 76.0 g of the compound carbon disulfide 1 c s 2 2 . In the
Nitella [24]

Answer is: mass of unused sulfur is 5.87 grams.

Balanced chemical reaction: C + 2S → CS₂.

m(C) = 12.0 g; mass of carbon.

m(S) = 70.0 g; mass of sulfur.

n(C) = m(C) ÷ M(C).

n(C) = 12 g ÷ 12 g/mol.

n(C) = 1 mol; amount of substance.

n(S) = m(S) ÷ M(S).

n(S) = 70 g ÷ 32.065 g/mol.

n(S) = 2.183 mol.

From chemical reaction: n(C) : n₁(S) = 1 : 2.

n₁(S) = 1 mol · 2 = 2 mol.

Δn(S) = n(S) - n₁(S).

Δn(S) = 2.183 mol - 2 mol.

Δn(S) = 0.183 mol; amount of unused sulfur.

Δm(S) = 0.183 mol · 32.065 g/mol.

Δm(S) = 5.87 g.

4 0
3 years ago
I need some help this is due soon
nikitadnepr [17]

Answer:

catalysts help speed up reactions which implies that they provide a alternative pathway and when there is less activation energy more particles have more energy to react

5 0
2 years ago
1Calculate the density of an object that has a mass of 84.7g and a volume of 59.3 cm3
Iteru [2.4K]

Answer:

<h2>1.43 g/cm³</h2>

Explanation:

The density of a substance can be found by using the formula

density =  \frac{mass}{volume} \\

From the question

mass = 84.7 g

volume = 59.3 cm³

We have

density =  \frac{84.7}{59.3}  \\  = 1.428330...

We have the final answer as

<h3>1.43 g/cm³</h3>

Hope this helps you

7 0
3 years ago
A gas cylinder contains 2.0 mol of gas X and 6.0 mol of gas Y at a total pressure of 2.1 atm. What is the partial pressure of ga
vivado [14]

Answer :  The partial pressure of X and Y gases are, 0.525 and 1.575 atm respectively.

Explanation : Given,

Moles of X = 2.0 mole

Moles of Y = 6.0 mole

Total pressure = 2.1 atm

Now we have to calculate the mole fraction of X and Y.

\text{Mole fraction of }X=\frac{\text{Moles of }X}{\text{Moles of }X+\text{Moles of }Y}

\text{Mole fraction of }X=\frac{2.0}{2.0+6.0}=0.25

and,

\text{Mole fraction of }Y=\frac{\text{Moles of }Y}{\text{Moles of }X+\text{Moles of }Y}

\text{Mole fraction of }Y=\frac{6.0}{2.0+6.0}=0.75

Now we have to calculate the partial pressure of X and Y.

According to the Raoult's law,

p_i=X_i\times p_T

where,

p_i = partial pressure of gas

p_T = total pressure of gas  = 2.1 atm

X_i = mole fraction of gas

p_{X}=X_{(X)}\times p_T

p_{X}=0.25\times 2.1atm=0.525atm

and,

p_{Y}=X_{(Y)}\times p_T

p_{Y}=0.75\times 2.1atm=1.575atm

Thus, the partial pressure of X and Y gases are, 0.525 and 1.575 atm respectively.

4 0
3 years ago
Read 2 more answers
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