All categories

4 years ago

What volume (in milliliters) of oxygen gas is required to react with 4.03 g of Mg at STP?

Chemistry

2 answers:

laiz [17]4 years ago

7 0

Answer:

1860

Explanation:

you round 1857 and get 1860

BigorU [14]4 years ago

6 0

Mg reaction with O₂ gas will produce MgO so the equation will be
2Mg+O₂⇒2MgO. (You have to find the equation in order two figure out the number of moles of O₂ that will react with 1 mole of MgO).

The first step is to find the number of moles of Mg in 4.03g of Mg. You can do this by dividing 4.03g Mg by its molar mass (which is 24.3g/mol) to get 0.1658mol Mg. Then you have to find the number of moles of O₂ that will react with 0.1658mol Mg. To do this you need to use the fact that 1mol O₂ will react with 2mol Mg (this reatio is from the chemical equation) so you have to multiply 0.1658mol Mg by (1mol O₂)/(2mol Mg) to get 0.0829mol O₂. From here you would usually use PV=nRT and solve for V However, the question tells us that we are at STP, that means you can use the fact that 22.4L of gas is 1 mol of gas at STP. Using that information we can find the volume of O₂ gas by mulitlying 0.0829mol O₂ by 22.4L/mol to get 1.857L which equals 1857mL.
therefore, 1857mL of O₂ gas will react with 4.03g of Mg.

I hope this helps. Let me know in the comments if anything is unclear.

You might be interested in

When hydrochloric acid is poured over potassium sulfide, 43.7 mLmL of hydrogen sulfide gas is produced at a pressure of 758 torr

kvasek [131]

Answer:

0.196 grams of K2S reacted

Explanation:

When hydrochloric acid is poured over potassium sulfide, 43.7 mLmL of hydrogen sulfide gas is produced at a pressure of 758 torrtorr and 26.0 ∘C

How much potassium sulfide has reacted in grams?

Step 1: Data given

Volume of hydrogen sulfide (H2S) produced = 43.7 mL

Pressure = 758 torr = 758/760 = 0.9973684 atm

Temperature = 26.0 °C = 273 + 26 = 299 K

Step 2: The balanced equation

2 HCl + K2S → H2S + 2 KCl

Step 3: Calculate moles H2S

p*V = nRT

n = (pV)/(RT)

⇒ with n= the number of moles of H2S

⇒ with p = the pressure = 0.9973684 atm

⇒ with V = the volume of the gas = 43.7 mL = 0.0437 L

⇒ with R = the gas constant = 0.08206 L*atm/K*mol

⇒ with T = The temperature = 26°C = 299 Kelvin

n = (0.9973684 * 0.0437)/ (0.08206*299)

n = 0.001776 moles H2S

Step 4: calculate moles of K2S

For 2 moles HCl we need 1 mol K2S to produce 1 mol H2S and 2 moles KCl

For 0.001776 moles H2S produced, we need 0.001776 moles K2S

Step 5: Calculate mass of K2S

Mass K2S = moles K2S * molar mass K2S

Mass K2S = 0.001776 moles * 110.26 g/mol

Mass K2S = 0.196 grams K2S

0.196 grams of K2S reacted

6 0

3 years ago

8. What is the molarity of a CsOH solution if 30.0 mL of the solution is neutralized by 26.4 mL 0.25 M HBr solution (Hint: Ma x

anyanavicka [17]

Answer:

Remember, Molarity is moles of solute divided by Liters of solution. ... Hint: Don't forget to convert mL to L and use the formula Ma x Va = Mb x Vb. You are ... 8 What is the molarity of a CsOH solution if 30.0 mL of the solution is neutralized by 26.4 mL 0.25 M HBr solution ( Hint: Ma x Va = Mb x Vb. Rearrange to solve for Mb )? ..

Explanation:

pls follow me

6 0

3 years ago

Read 2 more answers

HELP HURRRRYYY

LekaFEV [45]

I would say the answer is... <span>C. AgNO3 + LiOH AgOH + LiNO3
</span>
Good luck!!

5 0

3 years ago

Questions to be ask for testing a starch

ddd [48]

I'm assuming you're asking how to test for a starch,

To do so you do this thing called the "Iodine Test"
The potassium iodide aqueous solution will form this complex with starch to form a purplish-blue color.

However, watch out for the pH as hydrolysis of starch could occur to prevent the test from working out-- and the temperature as the greater it is, the less intense the color is

8 0

3 years ago

0. 300 moles of sodium nitrite are needed for a reaction

timofeeve [1]

Molar concentration is the ratio of the moles and the volume. The volume of the solution that is needed is

<h3>What is Molarity?</h3>

Molarity or the molar concentration is the proportion of the moles of the solute to the volume of the solution in liters.

Given,

The molar concentration of the solution = 0.450 mol/L

Moles of sodium nitrite = 0.300 moles

Volume is calculated as:

$\begin{aligned} \rm volume &= \rm \dfrac{moles}{molarity}\\\\&= \dfrac{0.300}{0.450}\\\\&= 0.666 \;\rm L\end{aligned}$

Therefore, 666 mL of volume is needed.

Learn more about molarity here:

brainly.com/question/12783142

#SPJ4

5 0

2 years ago