Chemistry How many moles are in 1kg ice/water?

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To determine the number of moles in 1 kg of ice or water, first convert the mass from kilograms to grams, resulting in 1000 g. The molar mass of water (H2O) is 18 g/mol, so dividing 1000 g by 18 g/mol yields approximately 55.55 moles. This calculation shows that 1 kg of water or ice contains 55.55 moles of H2O. The process involves simple unit conversion and application of the molar mass ratio. Understanding these steps is essential for solving similar molar mass problems.
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How many moles are in 1kg ice/water?
 
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This is a very simple molar mass problem.

First, convert kg to g.
Then, multiply the number of grams by the mol/molar mass ratio. Use the molar mass of H2O.

Since grams will be being multiplied by #mols/grams, the grams cancel, leaving the number of mols in 1 kg of water/ice.
 
Here is another simple explanation:

First convert the mass in kg to g ( 1kg=1000g). Now 18g of H20 is equivalent to 1 mole. Hence, 1000g of it would be equal to 1000/18 moles. This comes out be 55.55 moles. Thus 1 kg of water or ice has 55.55 moles of H20.
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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