Ask question

Ask question

All categories

3 years ago

15

Delta H in chemistry means????

2 answers:

goblinko [34]3 years ago

3 0

In chemistry, the letter "H" represents the enthalpy of a system. Enthalpy refers to the sum of the internal energy of a system plus the product of the system's pressure and volume. The delta symbol is used to represent change. Therefore, delta H represents the change in enthalpy of a system in a reaction.

Papessa [141]3 years ago

3 0

Answer:

In chemistry, the letter "H" represents the enthalpy of a system

Explanation:

You might be interested in

Arrange the core steps of the scientific method in sequential order

Sloan [31]

HOMER - <span>hypothesize, operationalize, measure, evaluate, and replicate/revise/report."</span>

7 0

3 years ago

Read 2 more answers

A mole of the element U (uranium) and a mole of CO2

ElenaW [278]

<span>An equal number of particles. Hope this helps! :D</span>

4 0

3 years ago

Which scientist discovered that other galaxies and stars were moving away from us at speeds proportional to how far they were aw

julsineya [31]

I think it was edwin hubble but I'm not sure

7 0

3 years ago

A sample of water has a mass of 193 g. Salt is added to the water, and the final solution weighs 238 g. How much salt was added?

icang [17]

Answer:

45 g of salt was added

Explanation:

238g-193g=45g

3 0

3 years ago

The Henry's law constant (kH) for O2 in water at 20°C is 1.28e-3 mol/l atm. How many grams of O2 will dissolve in 3.5 L of H2O t

Sophie [7]

Answer : The mass of $O_2$ dissolved will be, 0.2365 grams

Explanation :

First we have to calculate the concentration of $O_2$ .

As we know that,

$C_{O_2}=k_H\times p_{O_2}$

where,

$C_{O_2}$ = concentration of $O_2$ = ?

$p_{O_2}$ = partial pressure of $O_2$ = 1.65 atm

$k_H$ = Henry's law constant = $1.28\times 10^{-3}mole/L.atm$

Now put all the given values in the above formula, we get:

$C_{O_2}=(1.28\times 10^{-3}mole/L.atm)\times (1.65atm)$

$C_{O_2}=2.112\times 10^{-3}mole/L$

The concentration of $O_2$ = $2.112\times 10^{-3}mole/L$

Now we have to calculate the moles of $O_2$

$\text{Moles of }O_2=\text{Concentration of }O_2\times \text{volume of solution}$

$\text{Moles of }O_2=(2.112\times 10^{-3}mole/L)\times (3.5L)=7.392\times 10^{-3}mole$

Now we have to calculate the mass of $O_2$

$\text{Mass of }O_2=\text{Moles of }O_2\times \text{Molar mass of }O_2$

$\text{Mass of }O_2=(7.392\times 10^{-3}mole)\times (32g/mole)=0.2365g$

Therefore, the mass of $O_2$ dissolved will be, 0.2365 grams

4 0

3 years ago