What is KUFCA? in science?

How many molecules are in 1.75 moles of Caco3?

saw5 [17]

Answer:

1.054 x 10²⁴ molecules

Explanation:

In order to convert moles of any given substance into a number of molecules, we need to use Avogadro's number, which states the number of molecules -or atoms, in the case of elements- present in one mol:

In one mol there are 6.023x10²³ molecules.

We now convert 1.75 moles into molecules:

1.75 mol * 6.023x10²³ molecules/mol = 1.05x10²⁴ molecules

5 0

3 years ago

While performing the assays for the LDH kinetics experiment, you will pipet 25ul of 250 ug/ml LDH into 975 ul of assay buffer (T

ArbitrLikvidat [17]

Answer:

6.25 μg/mL

Explanation:

When a dilution is made, the mass of the solute is conserved (Lavoiser's law), so the mass pipetted will be the mass in the assay. The mass is the concentration (C) multiplied by the volume (V). If the pipet solution is called 1, and the assay 2:

m1 = m2

C1*V1 = C2*V2

C1 = 250 μg/mL

V1 = 25 μL

V2 = 975 μL + 25 μL = 1000 μL (is the final volume of the assay after the addition of LDH)

250*25 = C2*1000

C2 = 6.25 μg/mL

6 0

3 years ago

Consider the following reaction at a high temperature. Br2(g) ⇆ 2Br(g) When 1.35 moles of Br2 are put in a 0.780−L flask, 3.60 p

UNO [17]

Answer : The equilibrium constant $K_c$ for the reaction is, 0.1133

Explanation :

First we have to calculate the concentration of $Br_2$ .

$\text{Concentration of }Br_2=\frac{\text{Moles of }Br_2}{\text{Volume of solution}}$

$\text{Concentration of }Br_2=\frac{1.35moles}{0.780L}=1.731M$

Now we have to calculate the dissociated concentration of $Br_2$ .

The balanced equilibrium reaction is,

$Br_2(g)\rightleftharpoons 2Br(aq)$

Initial conc. 1.731 M 0

At eqm. conc. (1.731-x) (2x) M

As we are given,

The percent of dissociation of $Br_2$ = $\alpha$ = 1.2 %

So, the dissociate concentration of $Br_2$ = $C\alpha=1.731M\times \frac{1.2}{100}=0.2077M$

The value of x = 0.2077 M

Now we have to calculate the concentration of $Br_2\text{ and }Br$ at equilibrium.

Concentration of $Br_2$ = 1.731 - x = 1.731 - 0.2077 = 1.5233 M

Concentration of $Br$ = 2x = 2 × 0.2077 = 0.4154 M

Now we have to calculate the equilibrium constant for the reaction.

The expression of equilibrium constant for the reaction will be :

$K_c=\frac{[Br]^2}{[Br_2]}$

Now put all the values in this expression, we get :

$K_c=\frac{(0.4154)^2}{1.5233}=0.1133$

Therefore, the equilibrium constant $K_c$ for the reaction is, 0.1133

7 0

3 years ago

What is the molarity of a solution of 14.0 g NH4Br in enough H2O to make 150 mL of solution?

kiruha [24]

The molarity of a solution equals to the mole number of the solute/the volume of the solution. For NH4Br, we know that the mole mass is 98. So the molarity is (14/98) mol /0.15 L=0.95 mol/L.

8 0

3 years ago

Read 2 more answers

When driving a truck,is fuel crucial?

Natali [406]

Answer:

The answer is yes.

Explanation:

When driving any type of motorized vehicle, fuel is importatn. Fuel is what it runs on, so without it it wouldn't run. With trucks a lot more is needed because trucks are bigger, and tend to carry more than a little car does.

6 0

3 years ago