If you had 100 ml of juice how many milliters would be fruit juice

What is the answer please help

snow_lady [41]

Answer:

type the question brainly, someone already answered

Explanation:

4 0

4 years ago

Please help me. 9 weeks almost over and I am struggling with chemistry. I missed a couple days of school and don’t know any of t

astra-53 [7]

I provided the work and answers below, sorry about the red font.

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hopefully my answer helps! ♡

if my answers helped you please tell me, therefore I know.. that I did them correctly or incorrectly. anyways, have a great day/night!

8 0

3 years ago

What is the independent variable of Smithers experience?

amm1812

Answer:

Smithers thinks that a special juice will increase the productivity of workers. He creates two groups of 50 workers each and assigns each group the same task (in this case, they're ... Group A is given the special juice to drink while they work. Group ... 1. Control Group. Group B. 2. Independent Variable. volume of special juice.

Explanation:

8 0

3 years ago

) B5H9(l) is a colorless liquid that will explode when exposed to oxygen. How much heat is released when 0.211 mol of B5H9 react

Tom [10]

Answer: The amount of heat released when 0.211 moles of $B_5H_9(l)$ reacts is 554.8 kJ

Explanation:

The chemical equation for the reaction of $B_5H_9$ with oxygen gas follows:

$2B_5H_9(l)+12O_2(g)\rightarrow 5B_2O_3(s)+9H_2O(l)$

The equation for the enthalpy change of the above reaction is:

$\Delta H_{rxn}=[(5\times \Delta H_f_{(B_2O_3(s))})+(9\times \Delta H_f_{(H_2O(l))})]-[(2\times \Delta H_f_{(B_5H_9(l))})+(12\times \Delta H_f_{(O_2(g))})]$

We are given:

$\Delta H_f_{(H_2O(l))}=-285.4kJ/mol\\\Delta H_f_{(B_2O_3(s))}=-1272kJ/mol\\\Delta H_f_{(B_5H_9(l))}=73.2kJ/mol\\\Delta H_f_{(O_2(g))}=0kJ/mol$

Putting values in above equation, we get:

$\Delta H_{rxn}=[(2\times (-1272))+(9\times (-285.4))]-[(2\times (73.2))+(12\times (0))]\\\\\Delta H_{rxn}=-5259kJ$

To calculate the amount of heat released for the given amount of $B_5H_9(l)$ , we use unitary method, we get:

When 2 moles of $B_5H_9(l)$ reacts, the amount of heat released is 5259 kJ

So, when 0.211 moles of $B_5H_9(l)$ will react, the amount of heat released will be = $\frac{5259}{2}\times 0.211=554.8kJ$

Hence, the amount of heat released when 0.211 moles of $B_5H_9(l)$ reacts is 554.8 kJ

7 0

3 years ago

Calculate the molar mass of Li2SO4.

asambeis [7]

Answer:

109.94 g/mol

Explanation:

Li is 6.94 and there's 2 of those = 13.88

1 S = 32.06

4 O = 63.996

Add all of those together to get 109.936 round to 109.94

3 0

3 years ago