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Alexxx [7]
3 years ago
12

What is the molar mass of KCI

Chemistry
1 answer:
9966 [12]3 years ago
7 0

Answer:

178.01347 ± 0.00093 g/mol

Explanation:

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How many liters of hydrogen gas are formed from the complete reaction of 1.04 mol of C? Assume that the hydrogen gas is collecte
Alisiya [41]

The volume is 2.23 liters of hydrogen gas.

<u>Explanation</u>:

                  moles of C = grams / molecular mass of C

                                     = 1.04 g / 12.011 g/mol.

                                     = 0.086

        The ratio between C and H2 is 1 : 1

                 moles H2 = 0.086

                               V = nRT / p

                                  = 0.086 x 0.08206 x 316 K / 1.0 atm

                              V  = 2.23 L.

8 0
3 years ago
How can chemical weathering contribute to physical weathering?
lora16 [44]

A-leads to the abrasion of rocks and minerals

A-dense vegetation cover

True

Explanation:

Weathering is the physical disintegration and chemical decomposition of rocks to form sediments and soils.

Agent of weathering are wind, water and glacier.

Chemical weathering contributes to physical weathering in that it leads to the abrasion of rocks and minerals.

During chemical weathering, a rock chemically combines with materials in the environment and weakens it.

When physical weathering processes are induced, grains produced independently weakening of bonds in rocks grind against one another and wears each other off.

An area with a dense vegetation cover undergoes rapid chemical weathering:

  • Plant roots penetrates deep into the rock and increases the surface area of chemical action.
  • Plants produce chemicals that combines with rocks and causes them to decay.
  • Since the area is always moist, chemical action becomes more severe.

Buildings and statues made of stone are subjected to the same degree of weathering as rocks exposed naturally.

This is true.

Statues and buildings weather just like rocks we find in nature.

It is the same sunshine and rain that impacts rocks that also impacts buildings and statues.

So they degrade at the same rate except they are protected.

learn more:

Erosion brainly.com/question/2473244

#learnwithBrainly

5 0
3 years ago
The following molecular equation represents the reaction that occurs when aqueous solutions of silver(I) nitrate and barium chlo
mrs_skeptik [129]

Answer:

Hey, I hope this helps. You gave the equation already balanced so there was no need to do so, the next thing we need to do after balancing is to split the strong electrolytes into ions. Once that is completed we cross off any reoccurring ions. That leaves us with our complete net ionic.

I also recommend you check out Wayne Breslyn on Yt. He is so helpful with equations like these.

5 0
2 years ago
When a person in the hospital is given fluids intravenously, the fluid is typically a saline (salt) solution with about the same
Sati [7]

Answer:

Swelling of the red blood cells occurs.

Explanation:

  • <u>Distilled water makes the blood hypotonic ,. that is a less concentrated solution, to the body  tissues including  the red blood cells. </u>
  • Therefore the water will enter the red blood cells and may cause them to lyse or swell.
  • <em>Additionally , water will enter the tissue spaces and cause sweling. </em>
  • But in the case of a hypertonic solution , ( a salt or saline solution ) , <em>This swelling does not happen because the concentration of the saline will be equal or more than the blood. </em>
  • Thus the water will flow only from the blood to the solution. <u>This will not cause swelling.</u>
  • But too much of salt is also not recommended.
5 0
3 years ago
The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1580 L of nitrogen gas and 351
ikadub [295]

Answer : The volume of reactant measured at STP left over is 409.9 L

Explanation :

First we have to calculate the moles of N_2 and H_2 by using ideal gas equation.

<u>For N_2 :</u>

PV_{N_2}=n_{N_2}RT

where,

P = Pressure of gas at STP = 1 atm

V = Volume of N_2 gas = 1580 L

n = number of moles N_2 = ?

R = Gas constant = 0.0821L.atm/mol.K

T = Temperature of gas at STP = 273 K

Putting values in above equation, we get:

1atm\times 1580L=n_{N_2}\times (0.0821L.atm/mol.K)\times 273K

n_{N_2}=70.49mole

<u>For H_2 :</u>

PV_{H_2}=n_{H_2}RT

where,

P = Pressure of gas at STP = 1 atm

V = Volume of H_2 gas = 3510 L

n = number of moles H_2 = ?

R = Gas constant = 0.0821L.atm/mol.K

T = Temperature of gas at STP = 273 K

Putting values in above equation, we get:

1atm\times 3510L=n_{H_2}\times (0.0821L.atm/mol.K)\times 273K

n_{H_2}=156.6mole

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

N_2(g)+3H_2(g)\rightarrow 2NH_3(g)

From the balanced reaction we conclude that

As, 3 mole of H_2 react with 1 mole of N_2

So, 156.6 moles of H_2 react with \frac{156.6}{3}\times 1=52.2 moles of N_2

From this we conclude that, N_2 is an excess reagent because the given moles are greater than the required moles and H_2 is a limiting reagent and it limits the formation of product.

Now we have to calculate the excess moles of N_2 reactant (unreacted gas).

Excess moles of N_2 reactant = 70.49 - 52.2 = 18.29 moles

Now we have to calculate the volume of reactant, measured at STP, is left over.

PV=nRT

where,

P = Pressure of gas at STP = 1 atm

V = Volume of gas = ?

n = number of moles of unreacted gas = 18.29 moles

R = Gas constant = 0.0821L.atm/mol.K

T = Temperature of gas at STP = 273 K

Putting values in above equation, we get:

1atm\times V=18.29mole\times (0.0821L.atm/mol.K)\times 273K

V=409.9L

Therefore, the volume of reactant measured at STP left over is 409.9 L

8 0
3 years ago
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