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olga2289 [7]
2 years ago
11

How many milligrams of AgNO3 is required to completely react with 81.5 mg LiOH?

Chemistry
1 answer:
BartSMP [9]2 years ago
7 0

Answer:

m_{AgNO_3}=577.6mg

Explanation:

Hello there!

In this case, according to the given chemical reaction, it is first necessary to compute the moles of reacting LiOH given its molar mass:

n_{LiOH}=81.5mg*\frac{1g}{1000mg}*\frac{1mol}{23.95g}  =0.0034molLiOH

Thus, since there is a 1:1 mole ratio between lithium hydroxide and silver nitrate (169.87 g/mol) the resulting milligrams turn out to be:

m_{ AgNO_3}=0.0034molLiOH*\frac{1molAgNO_3}{1molLiOH} *\frac{169.87gAgNO_3}{1molAgNO_3} *\frac{1000gAgNO_3}{1gAgNO_3} \\\\m_{AgNO_3}=577.6mg

Best regards!

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7 0
3 years ago
2131211.1994 x 102 mL<br> Scientific notation
andreyandreev [35.5K]

Answer:

The answer is 213121119.94. Please mark me brainliest if I helped.

7 0
3 years ago
***BRAINLIEST ASNWERRR***<br>How many grams are in 34.2 moles of Lithium (Li)?​
Step2247 [10]

Mass of Li = 237.38 g

<h3>Further explanation</h3>

The mole itself is the number of particles contained in a substance amounting to 6.02.10²³  

\large {\boxed {\boxed {\bold {mol = \frac {mass} {molar \: mass}}}}

<h3>Known</h3>

Moles of Li = 34.2

Molar mass(MW) of Li = 6.941 g/mol

then mass of Lithium (Li) :

\tt mol=\dfrac{mass}{MW}\\\\mass=mol\times MW\\\\mass=34.2\times 6,941~g/mol\\\\mass=\boxed{\bold{237.38~g}}

3 0
3 years ago
Assume prices increase from $15 to $18, yet quantity remains at 25. What is the total revenue?
UNO [17]

Given:

Number of items = 25

Price per item = $18

<u>To determine:</u>

The total revenue

<u>Explanation:</u>

Total revenue = quantity * price per item

                       = 25 items * 18 dollar/ 1 item = $450

Ans: A) The total revenue is $450

4 0
3 years ago
How much heat is released when 6.00 g of methane is combusted using the reaction below? CH4 + 2O2 ? CO2 + 2H2O ?Hrxn = -890. KJ
goblinko [34]

Answer : The amount of heat released is, -121.04 KJ

Solution : Given,

Enthalpy of reaction, \Delta H_{rxn} = -890 KJ

Mass of methane = 6 g

Molar mass of methane = 44 g/mole

First we have to calculate the moles of methane.

\text{Moles of methane}=\frac{\text{Mass of methane}}{\text{Molar mass of methane}}=\frac{6g}{44g/mole}=0.136moles

The given balanced reaction is,

CH_4+2O_2\rightarrow CO_2+2H_2O

From the balanced reaction we conclude that

1 mole of methane releases heat = -890 KJ

0.136 moles of methane releases heat = \frac{0.136moles}{1mole}\times -890KJ=-121.04KJ

Therefore, the amount of heat released is, -121.04 KJ

8 0
3 years ago
Read 2 more answers
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