All categories

3 years ago

Someone help What are the products in a chemical reaction?

Chemistry

2 answers:

Alisiya [41]3 years ago

7 0

Answer:

The substances that result from a chemical reaction.

Explanation:

The substances produced at the end of the reaction are known as the products.

Keith_Richards [23]3 years ago

3 0

Answer:

D) The substances that result in a chemical reaction.

In a chemical reaction the substances which takes part in it is called reactant and the result obtained is called product.

Catalyst are the substances which helps in increasing the chemical reaction

You might be interested in

A student needs to prepare 50.0 mL of a 1.20 M aqueous H2O2 solution. Calculate the volume of 4.9 M H2O2 stock solution that sho

Nonamiya [84]

Answer : The volume of 4.9 M $H_2O_2$ stock solution used to prepare the solution is, 12.24 ml

Solution : Given,

Molarity of aqueous $H_2O_2$ solution = 1.20 M = 1.20 mole/L

Volume of aqueous $H_2O_2$ solution = 50.0 ml = 0.05 L

(1 L = 1000 ml)

Molarity of $H_2O_2$ stock solution = 4.9 M = 4.9 mole/L

Formula used :

$M_1V_1=M_2V_2$

where,

$M_1$ = Molarity of aqueous $H_2O_2$ solution

$M_2$ = Molarity of $H_2O_2$ stock solution

$V_1$ = Volume of aqueous $H_2O_2$ solution

$V_2$ = Volume of $H_2O_2$ stock solution

Now put all the given values in this formula, we get the volume of $H_2O_2$ stock solution.

$(1.20mole/L)\times (0.05L)=(4.9mole/L)\times V_2$

By rearranging the term, we get

$V_2=0.01224L=12.24ml$

Therefore, the volume of 4.9 M $H_2O_2$ stock solution used to prepare the solution is, 12.24 ml

3 0

3 years ago

What is the name of the following chemical compound?

Lynna [10]

Answer: Dinitrogen pentoxide

Explanation:

5 0

2 years ago

Read 2 more answers

At 85°C, the vapor pressure of A is 566 torr and that of B is 250 torr. Calculate the composition of a mixture of A and B that b

Phantasy [73]

Answer:

Composition of the mixture:

$x_{A} =0.652=65.2$ %

$x_{B} =0.348=34.8$ %

Composition of the vapor mixture:

$y_{A} =0.809=80.9$ %

$y_{B} =0.191=19.1$ %

Explanation:

If the ideal solution model is assumed, and the vapor phase is modeled as an ideal gas, the vapor pressure of a binary mixture with $x_{A}$ and $x_{B}$ molar fractions can be calculated as:

$P_{vap}=x_{A}P_{A}+x_{B}P_{B}$

Where $P_{A}$ and $P_{B}$ are the vapor pressures of the pure compounds. A substance boils when its vapor pressure is equal to the pressure under it is; so it boils when $P_{vap}=P$ . When the pressure is 0.60 atm, the vapor pressure has to be the same if the mixture is boiling, so:

$0.60*760=P_{vap}=x_{A}P_{A}+x_{B}P_{B}\\456=x_{A}P_{A}+(1-x_{A})P_{B}\\456=x_{A}*(P_{A}-P_{B})+P_{B}\\\frac{456-P_{B}}{P_{A}-P_{B}}=x_{A}\\\\\frac{456-250}{566-250}=x_{A}=0.652$

With the same assumptions, the vapor mixture may obey to the equation:

$x_{A}P_{A}=y_{A}P$ , where P is the total pressure and y is the fraction in the vapor phase, so:

$y_{A} =\frac{x_{A}P_{A}}{P}=\frac{0.652*566}{456} =0.809=80.9$ %

The fractions of B can be calculated according to the fact that the sum of the molar fractions is equal to 1.

7 0

3 years ago

Which one is right for brainliest

SVEN [57.7K]

I believe it is the second option

6 0

2 years ago

Read 2 more answers

How many moles of helium is required to blow up a balloon to 87.1 liters at 74 C and 3.5 atm?

marshall27 [118]

Moles of helium is required to blow up a balloon to 87.1 liters at 74 C and 3.5 atm is 021.65 mole

Mole is the unit of amount of substances of specified elementary entities

According to the ideal gas law he number of moles of a gas n can be calculated knowing the partial pressure of a gas p in a container with a volume V at an absolute temperature T from the equation

n =pV/RT

Here given data is volume = 87.1 liters

Temperature = 74 °C means 347.15 k

Pressure = 3.5 atm

R = 0.0821

Putting this value in ideal gas equation then

n =pV/RT

n = 3.5 atm×87.1 liters / 0.0821 ×347.15 k

n = 021.65 mole

Moles of helium is required to blow up a balloon to 87.1 liters at 74 C and 3.5 atm is 021.65 mole

Know more about mole of helium

brainly.com/question/23365554

#SPJ1

8 0

9 months ago