Ask question

Ask question

All categories

3 years ago

7

To cook a steak to medium-rare, it needs to have an internal temperature of 135

1 answer:

Nady [450]3 years ago

7 0

t<135 because it will be less then 135°

You might be interested in

A doctor is testing a new medication and he doesn’t tell the people in the study about the possible side effects of the medicine

balu736 [363]

Answer: He is being non-compliant

3 0

3 years ago

Consider the reaction. 2 HBr(g) ¡ H2(g) + Br2(g) a. Express the rate of the reaction in terms of the change in concentration of

Studentka2010 [4]

Answer :

(A) The rate expression will be:

$Rate=-\frac{1}{2}\frac{d[HBr]}{dt}=+\frac{d[H_2]}{dt}=+\frac{d[Br_2]}{dt}$

(B) The average rate of the reaction during this time interval is, 0.00176 M/s

(C) The amount of Br₂ (in moles) formed is, 0.0396 mol

Explanation :

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

The given rate of reaction is,

$2HBr(g)\rightarrow H_2(g)+Br_2(g)$

The expression for rate of reaction :

$\text{Rate of disappearance of }HBr=-\frac{1}{2}\frac{d[HBr]}{dt}$

$\text{Rate of disappearance of }H_2=+\frac{d[H_2]}{dt}$

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

<u>Part A:</u>

The rate expression will be:

$Rate=-\frac{1}{2}\frac{d[HBr]}{dt}=+\frac{d[H_2]}{dt}=+\frac{d[Br_2]}{dt}$

<u>Part B:</u>

$\text{Average rate}=-\frac{1}{2}\frac{d[HBr]}{dt}$

$\text{Average rate}=-\frac{1}{2}\frac{(0.512-0.600)M}{(25.0-0.0)s}$

$\text{Average rate}=0.00176M/s$

The average rate of the reaction during this time interval is, 0.00176 M/s

<u>Part C:</u>

As we are given that the volume of the reaction vessel is 1.50 L.

$\frac{d[Br_2]}{dt}=0.00176M/s$

$\frac{d[Br_2]}{15.0s}=0.00176M/s$

$[Br_2]=0.00176M/s\times 15.0s$

$[Br_2]=0.0264M$

Now we have to determine the amount of Br₂ (in moles).

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

$\text{Moles of }Br_2=0.0264M\times 1.50L$

$\text{Moles of }Br_2=0.0396mol$

The amount of Br₂ (in moles) formed is, 0.0396 mol

8 0

3 years ago

What type of energy does a saxophone player have and what energy does it turn into

Serjik [45]

The energy it plays is heat energy ahahha an

3 0

4 years ago

What gas is formed when water is boild

Tom [10]

Water vapor
Its still water(H2O)
Just in the gas form

7 0

3 years ago

Read 2 more answers

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr. Determine the pH of the solution after the addition of 300.0 mL

Vera_Pavlovna [14]

Answer : The correct option is, (C) 1.7

Explanation :

First we have to calculate the moles of $Ca(OH)_2$ and $HBr$ .

$\text{Moles of }Ca(OH)_2=\text{Concentration of }Ca(OH)_2\times \text{Volume of solution}=0.10M\times 0.1L=0.01mole$

$\text{Moles of }HBr=\text{Concentration of }HBr\times \text{Volume of solution}=0.10M\times 0.3L=0.03mole$

The balanced chemical reaction will be:

$Ca(OH)_2+2HBr\rightleftharpoons CaBr_2+2H_2O$

0.01 mole of $Ca(OH)_2$ dissociate to give 0.01 mole of $Ca^{2+}$ ion and 0.02 mole of $OH^-$ ion

and

0.03 mole of $HBr$ dissociate to give 0.03 mole of $H^+$ ion and 0.03 mole of $Br^-$ ion

That means,

0.02 moles of $OH^-$ ion neutralize by 0.02 moles of $H^+$ ion.

The excess moles of $H^+$ ion = 0.03 - 0.02 = 0.01 mole

Total volume of solution = 100 + 300 = 400 ml = 0.4 L

Now we have to calculate the concentration of $H^+$ ion.

$\text{Concentration of }H^+=\frac{\text{Moles of }H^+}{\text{Total volume}}$

$\text{Concentration of }H^+=\frac{0.01mole}{0.4L}=0.025M$

Now we have to calculate the pH of the solution.

$pH=-\log [H^+]$

$pH=-\log (0.025M)$

$pH=1.7$

Therefore, the pH of the solution is, 1.7

5 0

3 years ago