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3 years ago

Can anyone help me with this since it is a quiz and I am really bad at chemistry!!

Chemistry

1 answer:

lord [1]3 years ago

5 0

Answer:

Down below <3

Explanation:

1. 1 $N_{2}$ + 3 $H_{2}$ ---> 2 $NH_{3}$

2. 2 $KClO_{3}$ ---> 2 KCl + 3 $O_{2}$

3. 1 $Na_{3}PO_{4}$ + 3 HCl ---> _ 3_ NaCl + 1 $H_{3}PO_{4}$

4. 1 $C_{2}H_{6}O$ + 3 $O_{2}$ ---> 2 $CO_{2}$ + 3 $H_{2}O$

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What volume of Co2 (carbon (iv) oxide)

hram777 [196]

Answer:

2.1056L or 2105.6mL

Explanation:

We'll begin by calculating the number of mole in 10g of Na2CO3. This can be obtained as follow:

Molar mass of Na2CO3 = (23x2) + 12 + (16x3) = 106g/mol

Mass of Na2CO3 = 10g

Mole of Na2CO3 =.?

Mole = mass /molar mass

Mole of Na2CO3 = 10/106

Mole of Na2CO3 = 0.094 mole

Next, we shall determine the number of mole CO2 produced by the reaction of 0.094 mole of Na2CO3. This is illustrated below:

Na2CO3 + 2HCl —> 2NaCl + H2O + CO2

From the balanced equation above,

1 mole of Na2CO3 reacted to produce 1 mole of CO2.

Therefore, 0.094 mole of Na2CO3 will also react to 0.094 mole of CO2.

Next, we shall determine the volume occupied by 0.094 mole of CO2 at STP. This is illustrated below:

1 mole of a gas occupy 22.4L at STP. This implies that 1 mole CO2 occupies 22.4L at STP.

Now, if 1 mole of CO2 occupy 22.4L at STP, then, 0.094 mole of CO2 will occupy = 0.094 x 22.4 = 2.1056L

Therefore, the volume of CO2 produced is 2.1056L or 2105.6mL

7 0

3 years ago

What element has the smallest atomic radius

Mariulka [41]

Helium has the smallest atomic radius® Α⇒Ω

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3 years ago

You have a mixture that contains 0.380 moles of Ne(g), 0.250 moles of He(g), and 0.500 moles CH4(g) at 400 K and 6.25 atm. What

Bas_tet [7]

Answer:

1.38 atm

Explanation:

Partial pressure of a gas = total pressure × mole fraction of that gas.

Mole fraction of a gas is moles of a gas ÷ total moles of all gases.

4 0

2 years ago

A sample of H2 gas (12.28 g) occupies 100.0 L at 400.0 K and 2.00 atm. A sample weighing 9.49 g occupies ________ L at 353 K and

lutik1710 [3]

Considering the ideal gas law, a sample weighing 9.49 g occupies 68.67 L at 353 K and 2.00 atm.

Ideal gases are a simplification of real gases that is done to study them more easily. It is considered to be formed by point particles, do not interact with each other and move randomly. It is also considered that the molecules of an ideal gas, in themselves, do not occupy any volume.

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of the gases:

P× V = n× R× T

In this case, you know:

P= 2 atm
V= ?
n= $9.49 gramsx\frac{1 mole}{2 grams} = 4.745moles$ being 2g/mole the molar mass of H2, that is, the amount of mass that a substance contains in one mole.
R= 0.082 $\frac{atmL}{molK}$
T= 353 K