How can you read a determine the masses

If the volume is decreased from 5.15L to

hichkok12 [17]

Answer:

Increase

Explanation:

Boyle's law states volume and pressure have an inverse relationship.

- Hope that helped! Let me know if you need further explanation.

3 0

3 years ago

What mass will 33.6 L of chlorine gas (Cl2) have at STP?

chubhunter [2.5K]

Answer:

The answer is D.) 106 g

I hope I helped! ^-^

4 0

2 years ago

Read 2 more answers

At what step of glycolysis one NADH+ H+ is formed?

ElenaW [278]

Answer:

During Glycolysis, there is one step where NADH + H+ is formed from NAD+ O F-6-P - F- 1,6-BP O PGAL – 1,3-BPGA O 2-PGA - PEP O 3-PGA → 2-PGA.

3 0

2 years ago

Consider the reaction 5 Br− (aq) + BrO3− (aq) + 6 H+ (aq) → 3 Br2 (aq) + 3 H2O (l) The average rate of consumption of Br− is 1.8

kaheart [24]

Answer : The average rate of consumption of $H^+$ during the same time interval is, 2.17 M/s

Explanation :

The general rate of reaction is,

$aA+bB\rightarrow cC+dD$

Rate of reaction : It is defined as the change in the concentration of any one of the reactants or products per unit time.

The expression for rate of reaction will be :

$\text{Rate of disappearance of A}=-\frac{1}{a}\frac{d[A]}{dt}$

$\text{Rate of disappearance of B}=-\frac{1}{b}\frac{d[B]}{dt}$

$\text{Rate of formation of C}=+\frac{1}{c}\frac{d[C]}{dt}$

$\text{Rate of formation of D}=+\frac{1}{d}\frac{d[D]}{dt}$

$Rate=-\frac{1}{a}\frac{d[A]}{dt}=-\frac{1}{b}\frac{d[B]}{dt}=+\frac{1}{c}\frac{d[C]}{dt}=+\frac{1}{d}\frac{d[D]}{dt}$

From this we conclude that,

In the rate of reaction, A and B are the reactants and C and D are the products.

a, b, c and d are the stoichiometric coefficient of A, B, C and D respectively.

The negative sign along with the reactant terms is used simply to show that the concentration of the reactant is decreasing and positive sign along with the product terms is used simply to show that the concentration of the product is increasing.

The given rate of reaction is,

$5Br^-(aq)+BrO_3^-(aq)+6H^+(aq)\rightarrow 3Br_2(aq)+3H_2O(l)$

The expression for rate of reaction :

$\text{Rate of disappearance of }Br^-=-\frac{1}{5}\frac{d[Br^-]}{dt}$

$\text{Rate of disappearance of }BrO_3^-=-\frac{d[BrO_3^-]}{dt}$

$\text{Rate of disappearance of }H^+=-\frac{1}{6}\frac{d[H^+]}{dt}$

$\text{Rate of formation of }Br_2=+\frac{1}{3}\frac{d[Br_2]}{dt}$

$\text{Rate of formation of }H_2O=+\frac{1}{3}\frac{d[H_2O]}{dt}$

As we are given:

$\frac{d[Br^-]}{dt}=1.81M/s$

Now we have to determine the average rate of consumption of $H^+$ during the same time interval.

As,

$-\frac{1}{5}\frac{d[Br^-]}{dt}=-\frac{1}{6}\frac{d[H^+]}{dt}$

or,

$-\frac{1}{6}\frac{d[H^+]}{dt}=-\frac{1}{5}\frac{d[Br^-]}{dt}$

$\frac{d[H^+]}{dt}=\frac{6}{5}\frac{d[Br^-]}{dt}$

$\frac{d[H^+]}{dt}=\frac{6}{5}\times (1.81M/s)$

$\frac{d[H^+]}{dt}=2.17M/s$

Thus, the average rate of consumption of $H^+$ during the same time interval is, 2.17 M/s

6 0

3 years ago

2. What process of chemical weathering can create rust?

Anika [276]

Answer:

Oxidation

Explanation:

4 0

2 years ago